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of 55 (U.G Chemistry)

VIKRAM DEB AUTONOMOUS COLLEGE

JEYPORE, KORAPUT, ODISHA

COURSE OF STUDIES

OF

BACHELOR DEGREE SCIENCE UNDER CBCS

Subject: CHEMISTRY

FROM ADMISSION BATCH 2019 ONWARD

Published by

VIKRAM DEB AUTONOMOUS COLLEGE JEYPORE, KORAPUT, ODISHA

Website: www.vikramdebcollege.ac.in


PROGRAMME LERNING OUT COME OF B.Sc. (CHEMISTRY) PROGRAMME The Programme enable students

To understand basic methodology of Science in general and Chemistry in

particular. The students will learn the important analytical and instrumental tools

used for practising Chemistry.

To understand basic facts and concepts of Chemistry and to intigrate

knowledge of other branches of science to solve problems of chemistry.

To develop the ability to apply the principles of chemistry to solve different

problems.

To appriciate the achivements of chemistry and to know the role of chemistry in

nature and in society.

To develop critical thinking skill and analytical reasoning skill.

To develop apparatus and chemical handling skills and handling of common

lab equipments .

To be exposed to different processes of industries and their application.

To develop the ability to communicate scientific information in written and oral

format.

To develop the ability to work in a team and apply basic ethical principles.


Course structure of UG Chemistry Honours

Semester Course Course Name Credits Total marks

I AECC-I AECC-I 04 100

C-I Inorganic Chemistry-I 04 75

C-I Practical Inorganic Chemistry-I Lab 02 25

C-II Physical Chemistry-I 04 75

C-II Practical Physical Chemistry-I Lab 02 25

GE-I GE-I 04 75

GE-I Practical GE-I Lab 02 25

22 400

AECC-II AECC-II 04 100

C-III Organic Chemistry-I 04 75

C-III Practical Organic Chemistry-I Lab 02 25

II C-IV Physical Chemistry-II 04 75

C-IV Practical Physical Chemistry-II 02 25

GE-II GE-II 04 75

GE-II Practical GE-II Lab 02 25

22 400

C-V Inorganic Chemistry-II 04 75

C-V Practical Inorganic Chemistry-II Lab 02 25

C-VI Organic Chemistry-II 04 75

C-VI Practical Organic Chemistry-II Lab 02 25

C-VII Physical Chemistry-III 04 75

III C-VII Practical Physical Chemistry-III Lab 02 25

GE-III GE-III 04 75


GE-III Practical GE-III Lab 02 25

SEC-I SEC-I 04 100

28 500

C-VIII Inorganic Chemistry-III 04 75

C-VIII Practical Inorganic Chemistry-III Lab 02 25

C-IX Organic Chemistry-III 04 75

C-IX Practical Organic Chemistry-III Lab 02 25

C-X Physical Chemistry-IV 04 75

IV C-X Practical Physical Chemistry-IV Lab 02 25

GE-IV GE-IV (Theory) 04 75

GE-IV Practical GE-IV (Practical) 02 25

SEC-II SEC-II 04 100

28 500 C-XI Organic Chemistry-IV 04 75

C-XI Practical Organic Chemistry-IV 02 25

C-XII Physical Chemistry-V 04 75

C-XII Practical Physical Chemistry-V 02 25

DSE-I DSE-I (Polymer Chemistry) 04 75

V DSE-I Practical DSE-I Lab 02 25

DSE-II DSE-II(Green Chemistry) 04 75

DSE-II Practical DSE-II Lab 02 25


24 400

C-XIII Inorganic Chemistry- IV 04 75

C-XIII Practical Inorganic Chemistry-IV 02 25

C-XIV Organic Chemistry-V 04 75

VI C-XIV Practical Organic Chemistry-V 02 25

DSE-III

DSE-III (Advanced Organic

Chemistry ) 04 75

DSE-III Practical DSE-III Lab 02 25

DSE-IV Dissertation 06 100*

24 400

TOTAL 148 2600

CHEMISTRY (HONOURS) : A student to complete B.Sc. programme with chemistry Hons. has to pass the following courses. Core Course – 14 papers ( Core-I to Core-XIV) Discipline Specific Elective – 4 papers (DSE –I to DSE –IV) Generic Elective - 4 Papers ( Two Papers of Physics and Two Papers of Mathematics ) Ability Enhancement Compulsory Course-I (AECC –I) Ability Enhancement Compulsory Course-II (AECC –II) Skill Enhancement Compulsory Course-I (SECC –I) Skill Enhancement Compulsory Course-II (SECC –II)


Mark Distribution

Course Dissertation Presentation Viva-Voce

Total

DSE-IV (Project) 60 20 20 100 Course Mid Sem End Sem Total AECC-I ,AECC-II ,SECC-I & SECC-II 20 80 100

Pattern for 60 mark End Sem Question Paper (Subject With Practical)

PART-I PART-II PART-III PART-IV TOTAL 1x8 = 8 (All are compulsory)

1.5x8 =12 (8 Out of 10)

2x8 = 16

(8 Out of 10)

6x4 =24

(4 Either or type)

60

Pattern for 25 mark Question Paper( Practical)

Experiment Record Viva voce Total 15 05 05 25

Course Mid Sem End Sem Practical Total Core Course I to XIV

and DSE-I , DSE-II & DSE- III

15

60

25

100


CORE PAPER-1

INORGANIC CHEMISTRY-I Course Learning Outcome:

To study different models of atom and to understand quantum mechanical

approach to atom. To understand periodic properties of elements with reference

to modern periodic table. To explain different types of bond formation (ionic and

covalent).To predict geometry of covalent molecule on the basis of hybridisation

and VSEPR theory. To understand the nature of bonding in metals. To develop

skills in titration and theory behind Acid-Base and Redox titration.

Unit-I

Atomic structure : Bohr’s theory, its limitations and atomic spectrum of hydrogen atom, Sommerfeld’s modification. Wave mechanics: de Broglie equation, Heisenberg’s Uncertainty Principle (time independent) and its significance, Derivation of Schrödinger’s wave equation (for hydrogen atom) in Cartesian coordinate, significance of ψ and ψ2. Normalized and orthogonal wave functions. Sign of wave functions; Setting of Schrödinger’s equation in polar coordinates (derivation not required), radial and angular wave functions for hydrogen atom. Radial and angular distribution curves; Shapes of s, p, d and f orbitals; Quantum numbers and their significance. Pauli’s Exclusion principle, Hund’s rule of maximum multiplicity, Aufbau’s principle and its limitations.

Unit-II

Periodicity of elements

Periodicity of Elements: s, p, d, f block elements, the long form of periodic table.

Detailed discussion of the following properties of the elements, with reference to

s & p-blocks. (a) Effective nuclear charge, shielding or screening effect, Slater rules, variation of effective nuclear charge in periodic table. (b) Atomic radii (van

der Waals) (c) Ionic and crystal radii. (d) Covalent radii (octahedral and

tetrahedral) (e) Ionization enthalpy, Successive ionization enthalpies and factors

affecting ionization energy. Applications of ionization enthalpy. (f) Electron gain

enthalpy, trends of electron gain enthalpy. (g) Electronegativity, Pauling’s/ Mulliken’s electronegativity scales. Variation of electronegativity with bond order, partial charge, hybridization. Sanderson’s electron density ratio.


Unit-III

Chemical bonding-I Ionic bond: General characteristics, types of ions, size effects, radius ratio rule

and its limitations. Packing of ions in crystals. Born-Landé equation with

derivation. Madelung constant, Born-Haber cycle and its application, Solvation

energy. (ii) Covalent bond: Valence Bond theory (Heitler-London approach).

Hybridization with suitable examples of linear, trigonal planar, square planar,

tetrahedral, trigonal bipyramidal and octahedral arrangements, equivalent and

non-equivalent hybrid orbitals, Resonance and resonance energy. Molecular

orbital theory. Molecular orbital diagrams of diatomic and simple polyatomic

molecules N2, O2, C2, B2, F2, CO, NO, and their ions (CO+, NO+, NO-). Unit-IV

Chemical bonding-II VSEPR theory, shapes of simple molecules and ions containing lone and bond

pairs of electrons, multiple bonding (σ and π bond approach) and bond lengths. Covalent character in ionic compounds, polarizing power and polarizability.

Fajan’s rules and consequences of polarization. Ionic character in covalent

compounds: Bond moment and dipole moment. Percentage ionic character from

dipole moment and electronegativity difference.

Metallic Bond: Qualitative idea of valence bond and band theories.

Semiconductors and insulators. (ii) Weak Chemical Forces: van der Waals

forces, ion-dipole forces, dipole-dipole interactions, induced dipole interactions,

Instantaneous dipole-induced dipole interactions. Repulsive forces, Hydrogen

bonding (theories of hydrogen bonding, valence bond treatment) Effects of

chemical force, melting and boiling points, solubility energetics of dissolution

process.

Oxidation-reduction: Redox equations, standard electrode potential and its applications to inorganic reactions. Principles involved in some volumetric analyses (iron and copper).

Recommended Text Books:

1. Lee J. D., Concise Inorganic Chemistry Wiley India, 5th Edn., 2008. 2. Huheey J. E., Keiter E. A. and Keiter R. L., Inorganic Chemistry – Principles of

structure and reactivity, , Pearson Education, 4th Ed. 2002. 3. Puri, Sharma, Kalia, Principles of Inorganic Chemistry, Vishal Pub. Co., 33rd ed.,

2017 4. Selected Topic in Inorganic Chemistry, S. Chand, New Delhi, 17th Ed., 2010. 5. R.D.Madan, Advanced Inorganic Chemistry ,S.Chand New Delhi


Reference books

6. Das Asim K., Fundamentals of Inorganic Chemistry, Vol. I, CBS Publications, 2nd Ed. 2010.

7. Pradeep’s Inorganic Chemistry, Vol. I & II, Universal Book seller, 14th Ed. 2017.

CORE PAPER I LAB (A) Acid-Base Titrations

i. Estimation of carbonate and hydroxide present together in mixture. ii. Estimation of carbonate and bicarbonate present together in a mixture. iii. Estimation of free alkali present in different soaps/detergents

(B) Oxidation-Reduction Titrimetry

i. Standardization of KMnO4 with standard sodium oxalate and estimation of Fe(II) using standardized KMnO4 solution.

ii. Estimation of percentage of oxalic acid and sodium oxalate in a given mixture.

iii. Estimation of Fe(II) and Fe(III) in a mixture by standard K2Cr2O7 solution. Reference text:

1. Mendham, J., A. I. Vogel’s Quantitative Chemical Analysis 6th Ed., Pearson, 2009.

2. Gulati Shikha , Sharma Gulati JL and ManochaShagun, Practical Inorganic Chemistry, 1stEdn., CBS Publishers & Distributors Pvt Ltd., (2017).

CORE PAPER II

PHYSICAL CHEMISTRY- I

Course Learning Outcome: To understand the properties of gaseous and liquid state on the basis of Kinetic theory and to study structure of different solid. To study ionic equilibrium with reference to salt hydrolysis , buffer solution and theories of indicator. To develop skills for determination of viscosity and surface tension of liquid by using simple equpiments.

Unit-I Gaseous state-I Kinetic molecular model of a gas: postulates and derivation of the kinetic gas

equation; collision frequency; collision diameter; mean free path and viscosity of

gases, including their temperature and pressure dependence, relation between

mean free path and coefficient of viscosity, calculation of σ from η; variation of

viscosity with temperature and pressure. Maxwell distribution and its use in evaluating molecular velocities (average, root mean square and most probable) and average kinetic energy, law of equipartition of energy, degrees of freedom and molecular basis of heat capacities. Behaviour of real gases: Deviations from ideal gas behaviour, compressibility

factor, Z, and its variation with pressure for different gases. Causes of deviation

from ideal behaviour. van der Waal’s equation of state, its derivation and


application in explaining real gas behaviour. Isotherms of real gases and their

comparison with van der Waals isotherms, continuity of states, critical state,

relation between critical constants and van der Waals constants, law of

corresponding states.

Unit-II Liquid state Qualitative treatment of the structure of the liquid state; physical properties of

liquids; vapour pressure, surface tension and coefficient of viscosity, and their

determination. Effect of addition of various solutes on surface tension and

viscosity. Explanation of cleansing action of detergents. Temperature variation of

viscosity of liquids and comparison with that of gases. Qualitative discussion of

structure of water.

Ionic equilibria- I Strong, moderate and weak electrolytes, degree of ionization, factors affecting degree of ionization, ionization constant and ionic product of water. Ionization of weak acids and bases, pH scale, common ion effect; dissociation constants of mono- and diprotic acids.

Unit- III: Solid state

Nature of the solid state, law of constancy of interfacial angles, law of rational

indices, Miller indices, elementary ideas of symmetry, symmetry elements and

symmetry operations, seven crystal systems and fourteen Bravais lattices; X-ray

diffraction, Bragg’s law, a simple account of rotating crystal method and powder

pattern method. Analyses of powder diffraction patterns of NaCl, CsCl and KCl.

Defects in crystals (stoichiometric and non- stoichiometric). Glasses and liquid

crystals. Unit-IV

Ionic equilibria - II Salt hydrolysis-calculation of hydrolysis constant, degree of hydrolysis and pH for

different salts. Buffer solutions; derivation of Henderson equation and its

applications; buffer capacity, buffer range, buffer action and applications of

buffers in analytical chemistry and biochemical processes in the human body.

Solubility and solubility product of sparingly soluble salts – applications of

solubility product principle. Qualitative treatment of acid – base titration curves

(calculation of pH at various stages). Theory of acid–base indicators; selection of

indicators and their limitations. Multistage equilibria in polyelectrolyte systems;

hydrolysis and hydrolysis constants.



1. Atkins P. W. & Paula, J. de, Elements of Physical Chemistry, Oxford University Press, 6th Ed., (2006).

2. Puri, Sharma &Pathania, Principles of Physical Chemistry, Vishal Publishing Co, 47th Edn., 2017.

3. Kapoor K. L., Text Book of Physical Chemistry, McGraw Hill, 3rd Edn. 2017 4. Castellan G. W. Physical Chemistry 4thEdn. Narosa (2004).

Reference Books:

1. Kheterpal S.C., Pradeep’s Physical Chemistry, Vol. I & II, Pradeep Publications

2. Mortimer R. G., Physical Chemistry, Elsevier (Academic Press), 3rd Ed (2008).

3. Ball D. W. Physical Chemistry Thomson Press, India (2007). 4. Engel T. & Reid P., Physical Chemistry, 3rd Ed. Pearson (2013)

CORE PAPER II LAB

Surface tension measurements.

a. Determine the surface tension by (i) drop number (ii) drop weight method. b. Study the variation of surface tension of detergent solutions with

concentration. Viscosity measurement using Ostwald’s viscometer.

a. Determination of viscosity of aqueous solutions of (i) polymer (ii) ethanol and (iii) sugar at room temperature.

b. Study the variation of viscosity of sucrose solution with the concentration of solute.

Ionic equilibria a. Determination of solubility product of PbI2 by titrimetric method.

Reference Books

1. Khosla, B. D.; Garg, V. C. & Gulati, A. Senior Practical Physical Chemistry, R. Chand & Co., New Delhi (2011).

2. Garland, C. W.; Nibler, J. W. & Shoemaker, D. P. Experiments in Physical

Chemistry, 8th Ed.; McGraw-Hill, New York (2003).

3. Viswanathan, B., Raghavan, P.S. Practical Physical Chemistry, Viva Books (2009).


CORE PAPER – III ORGANIC CHEMISTRY - I

Course Learning Outcome: To understand the basics of organic chemistry and steriochemistry with reference to conformational and configurational isomerism. To understand the preperation and properties of alkanes , alkenes , alkynes and cycloalkanes. To develop the skills required for separation and purification of organic compounds.

Unit –I:

Basics of organic chemistry Electronic Displacements: Inductive, electromeric, resonance and mesomeric effects, hyperconjugation and their applications; Dipole moment; Organic acids and bases; their relative strength. Homolytic and heterolytic fission with suitable examples. Curly arrow rules; Electrophiles and Nucleophiles; Nucleophilicity and basicity; Types, shape and relative stability of carbocations, carbanions, free radicals and carbenes. Introduction to types of organic reactions and their mechanism: Addition, Elimination and Substitution reactions. Carbon-carbon sigma bonds Chemistry of alkanes: Formation of alkanes, Wurtz Reaction, Wurtz-Fittig Reactions, Free radical substitutions: Halogenation -relative reactivity and selectivity.

Unit – II:

Stereochemistry Fischer Projection, Newmann and Sawhorse Projection formulae; Geometrical isomerism: cis– trans and, syn-anti isomerism E/Z notations with C.I.P rules. Optical Isomerism: Optical Activity, Specific Rotation, Chirality/Asymmetry, Enantiomers, Molecules with one and two chiral-centres, Distereoisomers, meso-structures, Racemic mixture and resolution, inversion. Relative and absolute configuration: D/L and R/S designations.

Unit – III:

Chemistry of aliphatic hydrocarbons Carbon-Carbon pi bonds: Formation of alkenes and alkynes by elimination reactions, Mechanism of E1, E2, E1cb reactions. Saytzeff and Hofmann eliminations. Reactions of alkenes: Electrophilic additions their mechanisms (Markownikoff/ Anti Markownikoff addition), mechanism of oxymercuration-demercuration, hydroboration oxidation, ozonolysis, reduction (catalytic and chemical), syn and


anti-hydroxylation (oxidation). 1,2- and 1,4-addition reactions in conjugated dienes and, Diels-Alder reaction; Reactions of alkynes: Acidity, Electrophilic and Nucleophilic additions. Hydration to form carbonyl compounds, Alkylation of terminal alkynes.

Cycloalkanes and Conformational Analysis Types of cycloalkanes and their relative stability, Baeyer strain theory, Conformational analysis of alkanes (ethane and n-butane): Relative stability with energy diagrams. Energy diagrams of cyclohexane: Chair, Boat and Twist boat forms.

Unit – IV:

Aromatic hydrocarbons Aromaticity: Hückel’s rule, aromatic character of arenes, cyclic carbocations/carbanions and heterocyclic compounds with suitable examples.

Electrophilic aromatic substitution: halogenation, nitration, sulphonation and

Friedel-Craft’s alkylation/acylation with their mechanism. Directing effects of the

groups

Recommended Text Books: 1. Morrison, R. N. & Boyd, R. N., Organic Chemistry, Dorling Kindersley (India) Pvt.

Ltd. (Pearson Education). 2. Bhal and Bhal, Advanced Organic Chemistry, 2nd Edition, S. Chand Publisher,

2012.

3. Kalsi, P. S., Stereochemistry Conformation and Mechanism; 8thEdn, New Age International, 2015.

Reference Books:

1. Graham Solomons T. W., Fryhle, Craig B., Snyder Scott A, Organic Chemistry, Wiley Student Ed, 11th Edition (2013)

2. Jonathan Clayden, Nick Greeves, Stuart Warren, Organic Chemistry, 2nd Edition, Oxford Publisher, 2014.

3. Dhawan, S.N., Pradeep’s Organic Chemistry, (Vol. I and II), Pradeep

Publications


CORE PAPER III LAB

Students are required to learn the followings:

1. Checking the calibration of the thermometer

2. Determination of melting point, effect of impurities on the melting point – mixed melting point of two unknown organic compounds

3. Determination of boiling point of liquid compounds [boiling point lower than and

more than 100°C (up to 160°C) by distillation and capillary method, respectively](e.g., ethanol, cyclohexane, ethyl methyl ketone, cyclohexanone, acetylacetone, anisole, crotonaldehyde, mesityl oxide etc.).

List of experiments 1. Functional group tests for alcohols, phenols, carbonyl and carboxylic acid groups

and identification of unknown organic compounds of CHO system (without element detection).

2. Separation and purification of any one component of following binary solid mixture based on the solubility in common laboratory reagents like water (cold, hot), dil. HCl, dil. NaOH, dil. NaHCO3, etc. and determination of melting point.

Benzoic acid/p-Toluidine; p-Nitrobenzoic acid/p-Aminobenzoic acid; p-Nitrotolune/p-Anisidine etc.

3. Chromatography

• Separation of a mixture of two amino acids by ascending and horizontal paper chromatography

• Separation of a mixture of two sugars by ascending paper chromatography

OR

• Separation of a mixture of o-and p-nitrophenol or o-and p-aminophenol by thin layer chromatography (TLC)

Reference Books

1. Mann, F.G. & Saunders, B.C. Practical Organic Chemistry, Pearson Education (2009)

2. Furniss, B.S.; Hannaford, A.J.; Smith, P.W.G.; Tatchell, A.R. Practical Organic

Chemistry, 5th Ed., Pearson (2012)


CORE PAPER IV

PHYSICAL CHEMISTRY II

Course Learning Outcome: To understand the concepts of thermodynamics with reference to Enthalpy , Entropy , Free energy , Chemical potential and chemical equilibrium. To develop skills for use of equipments like pH meter and conductivity meter.and to perform thermal experiments using calorimeter.

Unit-I:

Chemical thermodynamics Intensive and extensive variables; state and path functions; isolated, closed and open systems; zeroth law of thermodynamics. First law: Concept of heat, q, work, w, internal energy, U, and statement of first law; enthalpy, H, relation between heat capacities, calculations of q, w, U and H for reversible, irreversible and free expansion of gases (ideal and van der Waals) under isothermal and adiabatic conditions. Thermochemistry: Heats of reactions: standard states; enthalpy of formation of molecules and ions and enthalpy of combustion and its applications; calculation of bond energy, bond dissociation energy and resonance energy from thermochemical data, effect of temperature (Kirchhoff’s equations) and pressure on enthalpy of reactions.

Unit-II

Carnot cycle, efficiency of heat engine, Carnot theorem Second Law: Concept of entropy; thermodynamic scale of temperature, statement of the second law of thermodynamics; molecular and statistical interpretation of entropy. Calculation of entropy change for reversible and irreversible processes. Third Law: Statement of third law, concept of residual entropy, calculation of absolute entropy of molecules. Free Energy Functions: Gibbs and Helmholtz energy; variation of S, G, A with T,

V, P; Free energy change and spontaneity. Relation between Joule-Thomson

coefficient and other thermodynamic parameters, inversion temperature, Gibbs-Helmholtz equation, Maxwell relations, thermodynamic equation of state.

Unit-III

Systems of variable composition Partial molar quantities, dependence of thermodynamic parameters on composition; Gibbs Duhem equation, chemical potential of ideal mixtures, change in thermodynamic functions in mixing of ideal gases.


Chemical equilibrium Criteria of thermodynamic equilibrium, degree of advancement of reaction, chemical equilibria in ideal gases, concept of fugacity. Thermodynamic derivation of relation between Gibbs free energy of reaction and reaction quotient (vant Hoff’s reaction). Equilibrium constants and their quantitative dependence on temperature, pressure and concentration. Free energy of mixing and spontaneity; thermodynamic derivation of relations between the various equilibrium constants Kp, Kc and Kx. Le Chatelier principle (quantitative treatment) and its applications.

Unit-IV

Solutions and Colligative Properties Dilute solutions; lowering of vapour pressure, Raoult’s and Henry’s Laws and

their applications. Thermodynamic derivation using chemical potential to derive relations between the four colligative properties: (i) relative lowering of vapour

pressure, (ii) elevation of boiling point, (iii) Depression of freezing point, (iv)

osmotic pressure and amount of solute. Applications in calculating molar masses

of normal, dissociated and associated solutes in solution. Recommended Text Books:


2. Principles of Physical Chemistry, Puri, Sharma &Pathania, Vishal Publishing Co, 47th Edn., 2017.

3. Text Book of Physical Chemistry, K. L. Kapoor, Mac Grow Hill, 3rdEdn. 2017 4. Castellan G. W. Physical Chemistry 4th Ed. Narosa (2004).

Reference Books:

1. Engel T. & Reid P., Physical Chemistry 3rd Ed. Pearson (2013). 2. McQuarrie, D. A. & Simon, J. D. Molecular Thermodynamics Viva Books Pvt.

Ltd.: New Delhi (2004). 3. Kheterpal S.C., Pradeep’s Physical Chemistry, Vol. I & II, Pradeep Publications.


CORE PAPER IV LAB

THERMOCHEMISTRY / PH -METRY a) Determination of heat capacity of a calorimeter for different volumes using change

of enthalpy data of a known system (method of back calculation of heat capacity of calorimeter from known enthalpy of solution or enthalpy of neutralization).

b) Determination of heat capacity of the calorimeter and enthalpy of neutralization of

hydrochloric acid with sodium hydroxide.

c) Calculation of the enthalpy of ionization of ethanoic acid.

d) Determination of heat capacity of the calorimeter and integral enthalpy (endothermic and exothermic) solution of salts.

e) Determination of basicity/proticity of a polyprotic acid by the thermochemical

method in terms of the changes of temperatures observed in the graph of temperature versus time for different additions of a base. Also calculate the enthalpy of neutralization of the first step.

f) Determination of enthalpy of hydration of copper sulphate.

g) Determination of heat of solution (∆H) of oxalic acid/benzoic acid from solubility

measurement. h). Study the effect on pH of addition of HCl/NaOH to solutions of acetic acid, sodium acetate and their mixtures. i). Preparation of buffer solutions of different pH (i) Sodium acetate-acetic acid (ii) Ammonium chloride-ammonium hydroxide

j) pH metric titration of (i) strong acid vs. strong base, (ii) weak acid vs. strong base.

k) Determination of dissociation constant of a weak acid.

Reference Books

1. Khosla, B. D.; Garg, V. C. & Gulati, A., Senior Practical Physical Chemistry, R. Chand & Co.: New Delhi (2011).

2. Athawale, V. D. & Mathur, P. Experimental Physical Chemistry, New Age

International: New Delhi (2001).

3. Viswanathan, B., Raghavan, P.S. Practical Physical Chemistry, Viva Books (2009)


CORE PAPER V

INORGANIC CHEMISTRY-II Course Learning Outcome: To understand the general principles of metallurgy and chemistry of s and p block elements including noble gases. To understand theories of acid and base and to explain preperation and properties of inorganic polymers. To develp skills for preperation of inorganic inorganic compounds and their application.

UNIT-I

General Principles of Metallurgy Chief modes of occurrence of metals based on standard electrode potentials.

Ellingham diagrams for reduction of metal oxides using carbon and carbon

monoxide as reducing agent. Electrolytic Reduction, Hydrometallurgy. Methods

of purification of metals: Electrolytic process, Parting process, van Arkel-de Boer

process and Mond’s process, Zone refining. Acids and Bases Brönsted-Lowry concept of acid-base reactions, solvated proton, relative strength of acids, types of acid-base reactions, Lewis acid-base concept, Classification of Lewis acids, Hard and Soft Acids and Bases (HSAB) Application of HSAB principle.

UNIT-II

Chemistry of s and p Block Elements - I Inert pair effect, Relative stability of different oxidation states, diagonal relationship and anomalous behaviour of first member of each group. Allotropy and catenation. Complex formation tendency of s and p block elements. Hydrides and their classification ionic, covalent and interstitial. Basic beryllium acetate and nitrate.

UNIT-III

Chemistry of s and p Block Elements - II Study of the following compounds with emphasis on structure, bonding, preparation, properties and uses. Boric acid and borates, boron nitrides, borohydrides (diborane) carboranes and

graphitic compounds, silanes. Oxides and oxoacids of nitrogen, Phosphorus and

chlorine. Peroxo acids of sulphur, interhalogen compounds, polyhalide ions,

pseudohalogens and basic properties of halogens.


UNIT-IV Noble Gases Occurrence and uses, rationalization of inertness of noble gases, clathrates; preparation and properties of XeF2, XeF4 and XeF6; Nature of bonding in noble gas compounds (Valence bond treatment and MO treatment for XeF2). Molecular shapes of noble gas compounds (VSEPR theory).

Inorganic Polymers:

Types of inorganic polymers, comparison with organic polymers, synthesis, structural aspects and applications of silicones and siloxanes. Borazines, silicates and phosphazenes, and polysulphates.


1. Lee J. D., Concise Inorganic Chemistry Wiley India, 5thEdn., 2008. 2. Huheey J. E., Keiter E. A. and Keiter R. L., Inorganic Chemistry – Principles of


2017. 4. Shriver D. E.,Atkins P. W., InorganicChemistry, Oxford University

Press,5thEdn.(2010). Reference books

1. Das Asim K., Fundamentals of Inorganic Chemistry, Vol. I, CBS Publications, 2nd Ed. 2010.


CORE PAPER V LAB

Iodometric / Iodimetric titrations (i) Standardization of sodium thiosulphate solution by standard of K2Cr2O7

solution. (ii) Estimation of Cu(II) using standard sodium thiosulphate solution

(Iodimetrically). (iii) Estimation of available chlorine in bleaching powder iodometrically.

Inorganic preparations

(i) Cuprous oxide (Cu2O) (ii) Cuprous chloride, Cu2Cl2 (iii) Manganese(III) phosphate, MnPO4.H2O (iv) Aluminium potassium sulphate K2SO4.Al2(SO4)2.24H2O (Potash alum). (v) Lead chromate (PbCrO4)

Reference Books: 1. Mendham, J., A. I. Vogel’s Quantitative Chemical Analysis, 6th Ed., Pearson,

2009. 2. Ahluwalia, V.K., Dhingra, S. and Gulati A, College Practical Chemistry, University

Press (2005). 3. Gulati Shikha , Sharma Gulati JL and ManochaShagun, Practical Inorganic

Chemistry, 1stEdn., CBS Publishers & Distributors Pvt. Ltd., (2017).


CORE PAPER VI ORGANIC CHEMISTRY-II

Course Learning Outcome: To understand preperation and properties of organic compounds like Alcohols , Phenols , Ethers ,Epoxides, Aldehydes, Ketones , Carboxylic acids and active methylene compounds. To develop the skills for preperation of different organic molecules.

UNIT-I Chemistry of Halogenated Hydrocarbons Alkyl halides: Methods of preparation, nucleophilic substitution reactions – SN1, SN2 and SNi mechanisms with stereochemical aspects and effect of solvent etc.; nucleophilic substitution vs. elimination. Aryl halides: Preparation, including preparation from diazonium salts, nucleophilic aromaticsubstitution; SNAr, Benzyne mechanism. Relative reactivity of alkyl, allyl/benzyl, vinyl and aryl halides towards nucleophilic substitution reactions. Organometallic compounds of Mg and Li – Use in synthesis of organic compounds.

UNIT-II

Alcohols, Phenols, Ethers and Epoxides Alcohols: preparation, properties and relative reactivity of 1°, 2°, 3° alcohols, Bouvaelt-BlancReduction; Preparation and properties of glycols: Oxidation by periodic acid and lead tetraacetate, Pinacol-Pinacolone rearrangement; Phenols: Preparation and properties; Acidity and factors effecting it, Ring substitutionreactions, Reimer–Tiemann and Kolbe’s–Schmidt Reactions, Fries and Claisen rearrangements with mechanism; Ethers and Epoxides: Preparation and reactions with acids. Reactions of epoxides withalcohols, ammonia derivatives and LiAlH4

UNIT-III

Carbonyl Compounds Structure, reactivity and preparation: Nucleophilic additions, Nucleophilic addition-elimination reactions with ammonia derivatives with mechanism; Mechanisms of Aldol and Benzoin condensation, Knoevenagel condensation, Perkin, Cannizzaro and Wittig reaction, Beckmann rearrangements,α haloform reaction and Baeyer Villiger oxidation, - substitution reactions, oxidations and reductions (Clemmensen, Wolff-Kishner, LiAlH4, NaBH4, MPV.; Addition reactions of unsaturated carbonyl compounds: Michael addition. Active methylene compounds: Keto-enol tautomerism. Preparation and synthetic applications of diethyl malonate and ethyl acetoacetate.


UNIT-IV

Carboxylic Acids and their Derivatives Preparation, physical properties and reactions of monocarboxylic acids: Typical reactions of dicarboxylic acids, hydroxy acids and unsaturated acids: succinic, lactic, malic, tartaric, citric, maleic and fumaric acids; Preparation and reactions of acid chlorides, anhydrides, esters and amides; Comparative study of nucleophilic sustitution at acyl group -Mechanism of acidic and alkaline hydrolysis of esters, Claisen condensation, Dieckmann and Reformatsky reactions, Hofmann-bromamide degradation and Curtius rearrangement.

Sulphur containing compounds: Preparation and reactions of thiols and thioethers.


1. Morrison, R. N. & Boyd, R. N., Organic Chemistry, Dorling Kindersley (India) Pvt. Ltd. (Pearson Education).

2. Bhal and Bhal, Advanced Organic Chemistry, 2nd Edition, S. Chand Publisher,

2012. 3. Mendham, J., A. I. Vogel’s Quantitative Chemical Analysis 6th Ed., Pearson,

2009.. Reference Books:


2. Jonathan Clayden, Nick Greeves, Stuart Warren, Organic Chemistry, 2nd

Edition, Oxford Publisher, 2014.

3. Dhawan, S.N., Pradeep’s Organic Chemistry, (Vol. I and II), Pradeep Publications

CORE PAPER VI LAB

Organic preparations:

i. Acetylation of one of the following compounds: amines (aniline, o-, m-, p-toluidines and o-, m-, p-anisidine) and phenols (β-naphthol, vanillin, salicylic acid) by any one method:

a. Using conventional method.

b. Using green approach

ii. Benzolyation of one of the following amines (aniline, o-, m-, p- toluidines and o-, m-, p-anisidine) and one of the following phenols (β-naphthol, resorcinol, p-cresol) by Schotten-Baumann reaction.

iii. Bromination of any one of the following:

a. Acetanilide by conventional methods b. Acetanilide using green approach (Bromate-bromide method)


iv. Nitration of any one of the following:

a. Acetanilide/nitrobenzene by conventional method

b. Salicylic acid by green approach (using ceric ammonium nitrate).

The above derivatives should be prepared using 0.5-1g of the organic compound.

Calculate percentage yield, based upon isolated yield (crude) and theoretical yield.

Purification of the crude product by recrystallisation from water/alcohol, or sublimation, whichever is applicable and determination of melting point.

Reference Books

1. Vogel, A. I. Elementary Practical Organic Chemistry, Part 1: Small scale

Preparations, Pearson (2011)


3. Furniss, B.S.; Hannaford, A.J.; Smith, P.W.G.; Tatchell, A.R. Practical

OrganicChemistry, 5th Ed., Pearson (2012) 4. Ahluwalia, V.K. & Aggarwal, R. Comprehensive Practical Organic

Chemistry:Preparation and Quantitative Analysis, University Press (2000).

5. Ahluwalia, V.K. & Dhingra, S. Comprehensive Practical Organic Chemistry: QualitativeAnalysis, University Press (2000).

CORE PAPER VII

PHYSICAL CHEMISTRY-III

UNIT-I

Phase Equilibria-I Concept of phases, components and degrees of freedom, derivation of Gibbs Phase Rule for nonreactive and reactive systems; Clausius-Clapeyron equation and its applications to solid-liquid, liquid-vapour and solid-vapour equilibria, phase diagram for one component systems, with applications (H2O and sulphur system). Phase diagrams for systems of solid-liquid equilibria involving eutectic (Pb-Ag system, desilverisation of lead), congruent (ferric chloride-water) and incongruent (sodium sulphate-water) melting points, completely miscible solid solutions (intermediate, medium, maximum freezing points).

UNIT-II Phase Equilibria-II Three component systems, water-chloroform-acetic acid system, triangular plots. Binary solutions: Gibbs-Duhem-Margules equation, its derivation and Applications to fractional distillation of binary miscible liquids (ideal and non-ideal), azeotropes, partial miscibility of liquids, CST, miscible pairs, steam distillation. Nernst distribution law: its derivation and applications.


UNIT-III

Chemical Kinetics Order and molecularity of a reaction, rate laws in terms of the advancement of a reaction, differential and integrated form of rate expressions up to second order reactions, experimental methods of the determination of orders. Kinetics of complex reactions (integrated rate expressions up to first order only): (i) Opposing reactions (ii) parallel reactions (iii) consecutive reactions and their differential rate equations (steady-state approximation in reaction mechanisms) (iv) chain reactions. Temperature dependence of reaction rates; Arrhenius equation; activation energy. Collision theory of reaction rates, qualitative treatment of the theory of absolute reaction rates.

UNIT-IV

Catalysis Types of catalyst, specificity and selectivity, mechanisms of catalyzed reactions at solid surfaces; effect of particle size and efficiency of nanoparticles as catalysts. Enzyme catalysis, Michaelis-Menten mechanism, acid-base catalysis. Surface chemistry: Physical adsorption, chemisorption, adsorption isotherms (Langmuir, Freundlich and Gibb’s isotherms), nature of adsorbed state.




3. Kapoor K. L., Text Book of Physical Chemistry, McGraw Hill, 3rd Edn. 2017 4. Castellan G. W. Physical Chemistry 4thEdn. Narosa (2004).

Reference Books: 1. Kheterpal S.C., Pradeep’s Physical Chemistry, Vol. I & II, Pradeep Publications 2. Levine, I. N. Physical Chemistry 6thEd., Tata McGraw-Hill (2011). 3. Ball D. W. Physical Chemistry Thomson Press, India (2007).

4. Engel T. & Reid P., Physical Chemistry 3rd Ed. Pearson (2013)

CORE PAPER VII LAB

1. Determination of distribution coefficients of:

(a) Iodine between water and carbon tetrachloride.

(b) Acetic/ benzoic acid between water and cyclohexane.

2. Study the equilibrium of at least one of the following reactions by the distribution method:

• I2 (aq) + I¯ → I3¯(aq)

• Cu2+(aq) + nNH3 → Cu(NH3)n


3. Study the kinetics of the following reactions.

(i) Integrated rate method: a) Acid hydrolysis of methyl acetate with hydrochloric acid. b) Saponification of ethyl acetate.

(ii) Compare the strengths of HCl and H2SO4 by studying kinetics of hydrolysis of methyl acetate.

4. Verify the Freundlich and Langmuir isotherms for adsorption of acetic acid on

activated charcoal. Reference Books:

1. Khosla, B. D.; Garg, V. C. & Gulati, A. Senior Practical Physical Chemistry, R. Chand & Co.: New Delhi (2011).

2. Garland, C. W.; Nibler, J. W. & Shoemaker, D. P. Experiments in Physical Chemistry8th Ed.; McGraw-Hill: New York (2003).

3. Halpern, A. M. &McBane, G. C. Experimental Physical Chemistry 3rdEd.; W.H. Freeman & Co.: New York (2003).

CORE PAPER VIII INORGANIC CHEMISTRY-III

UNIT-I

Coordination Chemistry Werner’s theory, valence bond theory (inner and outer orbital complexes), electroneutrality principle and back bonding. IUPAC nomenclature of coordination compounds, isomerism in coordination compounds. Stereochemistry of complexes with 4 and 6 coordination numbers. Chelate effect, Labile and inert complexes. Crystal field theory, measurement of CFSE weak and strong fields, pairing

energies, factors affecting the magnitude of 10 Dq in octahedral vs. tetrahedral

coordination, tetragonal distortions from octahedral geometry, Jahn-Teller theorem, square planar geometry. Qualitative aspect of ligand field and MO Theory.

UNIT-II

Transition Elements-I General group trends with special reference to electronic configuration, colour, variable valency, magnetic and catalytic properties, and ability to form complexes. Stability of various oxidation states and e.m.f. (Latimer &Bsworth

diagrams). Difference between the first, second and third transition series.


UNIT-III Transition Elements-II Chemistry of Ti, V, Cr Mn, Fe and Co in various oxidation states (excluding their metallurgy). Lanthanoids and Actinoids Electronic configuration, oxidation states, colour, spectral and magnetic properties,lanthanide contraction, separation of lanthanides (ion-exchange method only). General features of actinoids, separation of Np, Pm, Am from U.

UNIT-IV

Bioinorganic Chemistry Metal ions present in biological systems, classification of elements according to their action in biological system. Na/K-pump, carbonic anhydrase and

carboxypeptidase. Excess and deficiency of some trace metals. Toxicity of metal

ions (Hg, Pb, Cd and As), reasons for toxicity, Use of chelating agents in

medicine. Iron and its application in bio-systems, Haemoglobin and myoglobin.

Recommended Text Books: 1. Lee J. D., Concise Inorganic Chemistry, Wiley India, 5th Edn., 2008.

2. Huheey J. E., Keiter E. A. and Keiter R. L., Inorganic Chemistry – Principles of


2017. 4. Shriver D. E.,Atkins P. W., InorganicChemistry, Oxford University Press,5thEdn..

Reference books

1. Das Asim K., Fundamentals of Inorganic Chemistry, Vol. II, CBS Publications, 2nd Ed. 2010.

2. Bioinorganic Chemistry, Asim Kumar Das, Books & Allied (P) Ltd. 1st ed. 2015.

3. Selected Topic in Inorganic Chemistry, Mallick, Madan and Tuli, S. Chand Publisher. 17th Ed. 2010.


CORE PAPER VIII LAB Inorganic preparations Preparation of complexes: Hexamine nickel(II), [Ni(NH3)6]Cl2

Potassium trioxalatoferrate(III) trihydrate Tetraamminecopper(II) sulphate, [Cu(NH3)4]SO4.H2O Tetraamminecarbonatocobalt(III) nitrate

Complexometric titration

i. Estimation of Ca by EDTA ii. Estimation of Mg by EDTA


Gravimetric Analysis: i. Estimation of nickel(II) using dimethylglyoxime (DMG). ii. Estimation of copper as CuSCN

iii. Estimation of iron as Fe2O3 by precipitating iron as Fe(OH)3. iv. Estimation of Al(III) by precipitating with oxine and weighing as Al(oxine)3

(aluminiumoxinate).

Reference Books:

1. Vogel, A.I. A Textbook of Quantitative Inorganic Analysis, ELBS (1978). 2. Ahluwalia, V.K., Dhingra, S. and Gulati A, College Practical Chemistry, University

Press (2005). 3. Gulati Shikha , Sharma Gulati JL and ManochaShagun, Practical Inorganic

Chemistry, 1stEdn., CBS Publishers & Distributors Pvt Ltd., (2017).

CORE PAPER IX ORGANIC CHEMISTRY-III

UNIT-I

Nitrogen Containing Functional Groups Preparation and important reactions of nitro and compounds, nitriles. Amines: Effect of substituent and solvent on basicity; Preparation and properties:

Gabriel phthalimide synthesis, Carbylamine reaction, Mannich reaction, Hoffmann’s exhaustive methylation, Hofmann-elimination reaction; Distinction

between 1°, 2° and 3° amines with Hinsberg reagent and nitrous acid. UNIT-II

Diazonium Salts Preparation and their synthetic applications. Polynuclear Hydrocarbons Reactions of naphthalene and anthracene Structure, Preparation and structure elucidation and important derivatives of naphthalene and anthracene. Polynuclear hydrocarbons.

UNIT-III

Heterocyclic Compounds Classification and nomenclature, Structure, aromaticity in 5-numbered and 6-

membered rings containing one heteroatom; Synthesis, reactions and mechanism of substitution reactions of: Furan, Pyrrole (Paal-Knorr synthesis,

Knorr pyrrole synthesis, Hantzsch synthesis), Thiophene, Pyridine (Hantzsch

synthesis), Pyrimidine. Fischer indole synthesis and Madelung synthesis,

Derivatives of furan: Furfural and furoic acid (preparation only).


UNIT-IV

Alkaloids Natural occurrence, General structural features, Isolation and their physiological

action Hoffmann’s exhaustive methylation, Emde’s modification, Structure

elucidation and synthesis of Hygrine and Nicotine. Medicinal importance of Nicotine, Hygrine, Quinine, Morphine, Cocaine, and Reserpine. Terpenes Occurrence, classification, isoprene rule; Elucidation of structure and synthesis of Citral, Neral and α-terpineol.

Recommended Text Books: 1. Morrison, R. N. & Boyd, R. N., Organic Chemistry, Dorling Kindersley (India) Pvt.

Ltd. (Pearson Education). 2. Advanced Organic Chemistry, 2nd Edition, Arun Bahl & B S Bahl, S. Chand

Publisher, 2012. Reference Books:


2. Jonathan Clayden, Nick Greeves, Stuart Warren, Organic Chemistry, 2nd Edition,

Oxford Publisher, 2014.


CORE PAPER IX LAB Qualitative organic analysis of organic compounds

1. Detection of extra elements (N, X, S) in organic compounds by Lassaigne’s test.

2. Qualitative analysis of unknown organic compounds containing simple functional groups under CHN system (amine, nitro, amide and imide), determination of melting/boiling point, and preparation of their derivative.

Reference Books 1. Mann, F.G. & Saunders, B.C. Practical Organic Chemistry, Pearson Education

(2009) 2. Furniss, B.S.; Hannaford, A.J.; Smith, P.W.G.; Tatchell, A.R. Practical

OrganicChemistry, 5th Ed., Pearson (2012) 3. Ahluwalia, V.K. & Dhingra, S. Comprehensive Practical Organic

Chemistry:Qualitative Analysis, University Press (2000). 4. Ghoshal, A., Mahapatra, B., Nad, A. K. An Advanced Course in Practical

Chemistry, New Central Book Agency (2007).


CORE PAPER X PHYSICAL CHEMISTRY-IV

UNIT-I

Conductance-I Arrhenius theory of electrolytic dissociation. Conductivity, equivalent and molar

conductivity and their variation with dilution for weak and strong electrolytes.

Molar conductivity at infinite dilution. Kohlrausch law of independent migration of

ions. Debye-Hückel-Onsager equation, Wien effect, Debye-Falkenhagen effect, Walden’s rules.

UNIT-II

Conductance-II Ionic velocities, mobilities and their determinations, transference numbers and

their relation to ionic mobilities, determination of transference numbers using

Hittorf and Moving Boundary methods. Applications of conductance

measurement: (i) degree of dissociation of weak electrolytes, (ii) ionic product of

water (iii) solubility and solubility product of sparingly soluble salts, (iv)

conductometric titrations, and (v) hydrolysis constants of salts.

UNIT-III Electrochemistry-I Quantitative aspects of Faraday’s laws of electrolysis, rules of oxidation/reduction of ions based on half-cell potentials, applications of electrolysis in metallurgy and industry. Chemical cells, reversible and irreversible cells with examples. Electromotive force of a cell and its measurement, Nernst equation; Standard electrode (reduction) potential and its application to different kinds of half-cells. Application of EMF measurements in determining free energy, enthalpy and entropy of a cell reaction, (ii) equilibrium constants, and (iii) pH values, using hydrogen, quinone-hydroquinone, glass electrodes.

UNIT-IV

Electrochemistry-II Concentration cells with and without transference, liquid junction potential; determination of activity coefficients and transference numbers. Qualitative discussion of potentiometric titrations (acid-base, redox, precipitation). Electrical properties of atoms and molecules Basic ideas of electrostatics, Electrostatics of dielectric media. Clausius-Mosotti equation and Lorenz-Laurentz equation (no derivation), Dipole moment and molecular polarizabilities and their measurements.





3. Kapoor, K. L., Text Book of Physical Chemistry, Mac Grow Hill, 3rdEdn., 2017 4. Castellan G. W. Physical Chemistry 4th Ed. Narosa (2004).

Reference Books:

1. Engel T. & Reid P., Physical Chemistry 3rd Ed. Pearson (2013). 2. Levine, I. N. Physical Chemistry 6thEd., Tata McGraw-Hill (2011). 3. McQuarrie, D. A. & Simon, J. D. Molecular Thermodynamics Viva Books Pvt.

Ltd.: New Delhi (2004).

4. Kheterpal S.C., Pradeep’s Physical Chemistry, Vol. I & II, Pradeep Publications

CORE PAPER X LAB

Conductometry

I. Determination of cell constant. II. Determination of equivalent conductance, degree of dissociation and dissociation

constant of a weak acid. III. Perform the following conductometric titrations:

i. Strong acid vs. strong base ii. Weak acid vs. strong base iii. Strong acid vs. weak base

Potentiometry

I Perform the following potentiometric titrations:

i. Strong acid vs. strong base ii. Weak acid vs. strong base iii. Dibasic acid vs. strong base

Reference Books:

1. Khosla, B. D.; Garg, V. C. & Gulati, A., Senior Practical Physical Chemistry, R. Chand &Co.,New Delhi (2011).

2. Garland, C. W.; Nibler, J. W. & Shoemaker, D. P., Experiments in Physical

Chemistry8th Ed.; McGraw-Hill: New York (2003).

3. Halpern, A. M. &McBane, G. C., Experimental Physical Chemistry 3rdEd.; W.H. Freeman & Co., New York (2003).

4. Viswanathan, B., Raghavan, P.S., Practical Physical Chemistry, Viva Books

(2009).


CORE PAPER XI

ORGANIC CHEMISTRY-IV

UNIT-I

Organic Spectroscopy-I UV Spectroscopy: Types of electronic transitions, λmax, Lambert-Beer’s law and its limitations, Chromophores and Auxochromes,Bathochromic and Hypsochromic shifts, Intensity of absorption; Application of Woodward rules for calculation of λmax for the following systems: α,β the unsaturated aldehydes: ketones, carboxylic acids and esters; Conjugated dienes: alicyclic, homoannular and heteroannular; Extended conjugated systems (aldehydes, ketones and dienes); distinction between cis and trans isomers.

UNIT-II

Organic Spectroscopy-II IR Spectroscopy: Fundamental and non-fundamental molecular vibrations; IR

absorption positions of O and N containing functional groups; Effect of H-bonding, conjugation, resonance and ring size on IR absorptions; Fingerprint

region and its significance; application in simple functional group analysis. UNIT-III

Organic Spectroscopy-III NMR Spectroscopy: Basic principles of Proton Magnetic Resonance, chemical shift andfactors influencing it; Spin-spin coupling and coupling constant; Anisotropic effects in alkene, alkyne, aldehydes and aromatics; Interpretation of NMR spectra of simple compounds. Mass Spectroscopy- Basic principle, Fragmentation pattern, instrumentation, determination of m/e ratio. Application of mass spectroscopy on CH4, C2H6, n-butane and neo-pentane. Applications of IR, UV & NMR for identification of simple organic molecules.

UNIT-IV Carbohydrates Occurrence, classification and their biological importance. Monosaccharides: Constitution and absolute configuration of glucose and fructose, epimers and anomers, mutarotation, determination of ring size of glucose and fructose, Haworth projections and conformational structures; Interconversions of aldoses and ketoses; Killiani-Fischer synthesis and Ruff degradation; Disaccharides – Structure elucidation of maltose; Polysaccharides – Elementary treatment of starch, cellulose.


Recommended Text Books: 1. Kemp William, Organic Spectroscopy, 3rd Edition, Palgrave Publisher, 1991. 2. Davis, B. G., Fairbanks, A. J., Carbohydrate Chemistry, Oxford Chemistry

Primer, 3. J Kalsi P. S., Spectroscopy of Organic Compounds, 5th Edition, , New Age

International Publishers, 2016. 4. Advanced Organic Chemistry, 2nd Edition, Arun Bahl & B S Bahl, S. Chand

Publisher, 2012.

Reference Books: 1. Y R Sharma, Elementary Organic Spectroscopy, 5th Edition, S. Chand &

Company, 2013. 2. Jag Mohan, Organic Spectroscopy and Applications, NarosaPublishrs, 2012. 3. Graham Solomons T. W., Fryhle, Craig B., Snyder Scott A, Organic

Chemistry, Wiley Student Ed, 11th Edition (2013). 4. Jonathan Clayden, Nick Greeves, Stuart Warren, Organic Chemistry, 2nd

Edition, Oxford Publisher, 2014. 5. Dhawan, S.N., Pradeep’s Organic Chemistry, (Vol. I and II), Pradeep

Publications CORE PAPER XI LAB

1. Qualitative analysis of carbohydrate: aldoses and ketoses, reducing and non-reducing sugars.

2. Qualitative analysis of unknown organic compounds containing simple bifunctional groups, for e.g. salicylic acid, cinnamic acid, nitrophenols etc.

3. Quantitative estimation of sugars: (c) Estimation glucose by titration with Fehling’s solution. (d) Estimation of sucrose by titration with Fehling’s solution. (e) Estimation glucose and sucrose in a given mixture.

4. Identification of labelled peaks in the 1H NMR spectra of the known organic

compounds explaining the relative δ-values and splitting pattern.

5. Identification of labelled peaks in the IR spectrum of the same compound explaining the relative frequencies of the absorptions .

Reference Books:

1. Vogel, A.I. Quantitative Organic Analysis, Part 3, Pearson (2012).


3. Furniss, B.S.; Hannaford, A.J.; Smith, P.W.G.; Tatchell, A.R. Practical

OrganicChemistry, 5th Ed., Pearson (2012)

4. Ahluwalia, V.K. & Aggarwal, R. Comprehensive Practical Organic Chemistry:Preparation and Quantitative Analysis, University Press (2000).

5. Ahluwalia, V.K. & Dhingra, S. Comprehensive Practical Organic

Chemistry:Qualitative Analysis, University Press (2000).


CORE PAPER XII

PHYSICAL CHEMISTRY V

UNIT-I

Quantum Chemistry-I Quantum mechanical operators, Postulates of quantum mechanics, Schrödinger

equation and its application to particle in one-dimensional box (complete solution)

- quantization of energy levels, zero-point energy, normalization of wave

functions, probability distribution functions, nodal properties. Extension to three-dimensional boxes, separation of variables, degeneracy. Qualitative treatment of

simple harmonic oscillator model of vibrational motion: Setting up of Schrödinger

equation and discussion of solution and wave functions. Vibrational energy of

diatomic molecules and zero-point energy. Angular momentum: Commutation

rules, quantization of square of total angular momentum and z-component. Rigid rotator model of rotation of diatomic molecule: Schrödinger equation,

transformation to spherical polar coordinates. Separation of variables

(Preliminary treatment).

UNIT-II

Chemical Bonding Chemical bonding: Covalent bonding, valence bond and molecular orbital approaches, LCAO-MO treatment of H2

+. Bonding and antibonding orbitals. Qualitative extension to H2. Comparison of LCAO-MO and VB treatments of H2 (only wave functions, detailed solution not required) and their limitations. Localized and non-localized molecular orbitals treatment of triatomic (BeH2, H2O) molecules. Qualitative MO theory and its application to AH2 type molecules.

UNIT-III

Molecular Spectroscopy-I Interaction of electromagnetic radiation with molecules and various types of spectra; Born-Oppenheimer approximation. Rotation spectroscopy: Selection rules, intensities of spectral lines, determination of bond lengths of diatomic and linear triatomic molecules, isotopic substitution. Vibrational spectroscopy: Classical equation of vibration, computation of force constant, amplitude of diatomic molecular vibrations, anharmonicity, Morse potential, dissociation energies, fundamental frequencies, overtones, hot bands, degrees of freedom for polyatomic molecules, modes of vibration. Vibration-rotation spectroscopy: diatomic vibrating rotator, P, Q, R branches.


UNIT-IV

Molecular Spectroscopy-II Raman spectroscopy: Qualitative treatment of Rotational Raman effect; Effect of nuclear spin, Vibrational Raman spectra, Stokes and anti-Stokes lines; their intensity difference, rule of mutual exclusion. Electronic spectroscopy: Franck-Condon principle, electronic transitions, singlet and triplet states, fluorescence and phosphorescence, dissociation and predissociation.

Photochemistry Characteristics of electromagnetic radiation, physical significance of absorption

coefficients. Laws of photochemistry, quantum yield, actinometry, examples of low and

high quantum yields, photochemical equilibrium and the differential rate of

photochemical reactions, photosensitised reactions, quenching, chemiluminescence.


1. McQuarie D., Quantum Chemistry, University Science Publishers, 2007

2. Chandra, A. K. Introductory Quantum Chemistry Tata McGraw-Hill (2001).

3. Banwell, C. N. &McCash, E. M. Fundamentals of Molecular Spectroscopy 4th Ed. Tata McGraw-Hill: New Delhi (2010).

4. Prasad R K., Quantum Chemistry, New Age International Publishers, 4thEdn, 2010.

5. Rohatagi Mukherjee K K., Fundamentals of Photochemistry, Wiley Eastern Ltd., 1992.

Reference Books:


2. Kapoor, K. L., Text Book of Physical Chemistry, McGraw Hill, Vol. II, IV

3. Levine, I. N. Quantum Chemistry, PHI

CORE PAPER XII LAB

Spectroscopy/Colorimetry

1. Study of absorption spectra (visible range) of KMnO4 and determine the λmax value. Calculate the energies of the transitions in kJ mol-1, cm-1, and eV.

2. Verify Lambert-Beer’s law and determine the concentration of CuSO4/KMnO4/K2Cr2O7 in a solution of unknown concentration.

3. Determine the dissociation constant of an indicator (phenolphthalein).


Spectrophotometric titration

1. Determine the concentration of HCl against 0.1 N NaOH spectrophotometrically. 2. To find the strength of given ferric ammonium sulfate solution of (0.05 M) by using

EDTA spectrophotometrically.

3. To find out the strength of CuSO4 solution by titrating with EDTA spectrophotometrically.

4. To determine the concentration of Cu(II) and Fe(III) solution photometrically by

titrating with EDTA.

Reference Books

1. Khosla, B. D.; Garg, V. C. & Gulati, A., Senior Practical Physical Chemistry, R. Chand & Co.: New Delhi (2011).

2. Garland, C. W.; Nibler, J. W. & Shoemaker, D. P. Experiments in

PhysicalChemistry 8th Ed.; McGraw-Hill: New York (2003).

3. Halpern, A. M. &McBane, G. C. Experimental Physical Chemistry 3rdEd.; W.H. Freeman & Co.: New York (2003).

4. J. N. Gurtu, R. Kapoor, Experimental Physical Chemistry.

CORE PAPER XIII

INORGANIC CHEMISTRY-IV

UNIT-I

Organometallic Compounds-I

Definition and classification of organometallic compounds on the basis of bond type. Concept of hapticity of organic ligands. Metal carbonyls: 18 electron rule, electron count of mononuclear, polynuclear and substituted metal carbonyls of 3d series. General methods of preparation (direct combination, reductive carbonylation, thermal and photochemical decomposition) of mono and binuclear carbonyls of 3d series. Structures of mononuclear and binuclear carbonyls of Cr, Mn, Fe, Co and Ni using VBT. π-acceptor behaviour of CO (MO diagram of CO to be discussed), synergic effect and use of IR data to explain extent of back bonding. Zeise’s salt: Preparation and structure, evidences of synergic effect and comparison of synergic effect with that in carbonyls.


UNIT-II

Organometallic Compounds-II Metal Alkyls: Important structural features of methyl lithium (tetramer) and trialkyl

aluminium (dimer), concept of multicentre bonding in these compounds. Role of

triethylaluminium in polymerisation of ethene (Ziegler – Natta Catalyst). Species

present in ether solution of Grignard reagent and their structures. Ferrocene:

Preparation and reactions (acetylation, alkylation, metallation, Mannich Condensation), structure and aromaticity, comparison of aromaticity and

reactivity with that of benzene.

UNIT-III

Catalysis by Organometallic Compounds

Study of the following industrial processes and their mechanism:

1. Alkene hydrogenation (Wilkinson’s Catalyst)

2. Hydroformylation (Co salts)

3. Wacker Process

4. Synthetic gasoline (Fischer Tropsch reaction)

Theoretical Principles in Qualitative Analysis (H2S Scheme)

Basic principles involved in analysis of cations and anions and solubility products, common ion effect. Principles involved in separation of cations into groups and choice of group reagents. Interfering anions (fluoride and phosphate) and need to remove them after Group II.

UNIT-IV

Thermodynamic & kinetic aspects and reaction mechanism of metal complexes Thermodynamic and kinetic stability, Stepwise and overall formation constants and their relationship, factors affecting stability. Introduction to inorganic reaction mechanisms-types of reaction and classification od substitution reaction. Substitution reaction of square planar complexes, Trans effect and its applications, theories of trans-effect (electrostatic polarization and Static π-Bonding Theory). Kinetics of octahedral substitution (classification of metal ions based on water exchange rate), General mechanism of ligand substitution reactions in octahedral complexes (D, I, Id, Ia)



1. Huheey J. E., Keiter E. A. and Keiter R. L., Inorganic Chemistry – Principles of structure and reactivity, , Pearson Education, 4th Ed. 2002.

2. Puri, Sharma, Kalia, Principles of Inorganic Chemistry, Vishal Pub. Co., 33rd ed., 2017.

3. Shriver D. E.,Atkins P. W., InorganicChemistry, Oxford University Press,5thEdn.. 4. Svehla, G. Vogel's Qualitative Inorganic Analysis, 7th Edition, Prentice Hall,

1996-0307. Reference books


2. Selected Topic in Inorganic Chemistry, Mallick, Madan and Tuli, S. Chand

Publisher. 17th Ed. 2010.

3. Mehrotra R.C. and Singh, A. Organometallic Chemistry, New Age International Publishers, 2ndEdn, 2000.

4. Gupta B. D. and Elias A. J., Basic organometallic Chemistry, 2ndEdn., University Press (2013).

CORE PAPER XIII LAB

1. Qualitative analysis of mixtures containing 4 radicals (2 anions and 2 cations). Emphasis should be given to the understanding of the chemistry of different reactions. The following radicals are suggested:

CO32 -, NO2

-, S2-, SO32-, F-, Cl-, Br-, I-, NO3

-, PO43-, NH4

+, K+, Pb2+, Cu2+, Cd2+, Bi3+, Sn2+, Sb3+, Fe3+, Al3+,, Cr3+, Zn2+, Mn2+, Co2+, Ni2+, Ba2+, Sr2+, Ca2+, Mg2+. Mixtures may contain one insoluble component (BaSO4, SrSO4, PbSO4, CaF2 or Al2O3) Or combination of interfering anions e.g. CO3

2- and SO32-, NO2

- and NO3

-, Cl- and Br-, Cl-and I-, Br- and I-, NO3- and Br- , NO3

- and I-. 3.Spot tests should be done whenever possible.

Reference Books

1. Vogel’s Qualitative Inorganic Analysis, 7th Ed, Revised by G. Svehela, 4th Ed., Person (2007).

2. Gulati Shikha , Sharma Gulati JL and ManochaShagun, Practical Inorganic Chemistry, 1stEdn., CBS Publishers & Distributors Pvt Ltd., (2017).


CORE PAPER XIV ORGANIC CHEMISTRY-V

UNIT-I

Amino Acids, Peptides and Proteins Amino acids: Classification; α-Amino acids - Synthesis, ionic properties and reactions. Zwitter ions, pKa values, isoelectric point and electrophoresis. Peptides: Classification, determination of their primary structures-end group analysis, methods of peptide synthesis. Synthesis of peptides using N-protecting, C-protecting and activating groups -Solid-phase synthesis. Proteins: Structure of proteins, protein denaturation and renaturation

UNIT-II

Enzymes Introduction, classification and characteristics of enzymes. Salient features of

active site of enzymes. Mechanism of enzyme action (taking trypsin as example),

factors affecting enzyme action, coenzymes and cofactors and their role in

biological reactions, specificity of enzyme action (including stereo specificity),

enzyme inhibitors and their importance, phenomenon of inhibition (competitive,

uncompetitive and non-competitive inhibition including allosteric inhibition).

Nucleic Acids Components of nucleic acids, Nucleosides and nucleotides; Structure, synthesis and reactions of: Adenine, Guanine, Cytosine, Uracil and Thymine; Structure of polynucleotides.

UNIT-III

Lipids Introduction to oils and fats; common fatty acids present in oils and fats, Hydrogenntion of fats and oils, Saponification value, acid value, iodine number. Reversion and rancidity. Concept of Energy in Biosystems Cells obtain energy by the oxidation of foodstuff (organic molecules). Introduction to metabolism (catabolism and anabolism). Overview of catabolic pathways of fat and protein. Interrelationship in the metabolic pathways of protein, fat and carbohydrate. Caloric value of food, standard caloric content of food types.

UNIT-IV

Pharmaceutical Compounds: Structure and Importance Classification, structure and therapeutic uses of antipyretics: Paracetamol (with synthesis), Analgesics: Ibuprofen (with synthesis), Antimalarials: Chloroquine

(with synthesis). An elementary treatment of Antibiotics and detailed study of


chloramphenicol, Medicinal values of curcumin (haldi), azadirachtin (neem),

vitamin C and antacid (ranitidine).

Dyes Classification, colour and constitution; Mordant and Vat dyes; Chemistry of

dyeing. Synthesis and applications of: Azo dyes – Methyl orange and Congo red

(mechanism of Diazo Coupling); Triphenylmethane dyes - Malachite Green, and

crystal violet; Phthalein dyes – Phenolphthalein and Fluorescein.

Recommended Text books 1. Nelson, D.L., Cox, M.M. and Lehninger, A.L. Principles of Biochemistry. 6thEdn.

W.H. Freeman and Co. (2013).

2. Kar Ashutosh, Medicinal chemistry, New Age International (P) Ltd., (2007) 3. Debojyoti Das, Biochemistry, (part-I) Academic Publishers (1979)

Reference Books:

1. Talwar, G.P. & Srivastava, M. Textbook of Biochemistry and Human Biology, 3rd Ed. PHI Learning.

2. Berg, J.M., Tymoczko, J.L. &Stryer, L. Biochemistry, W.H. Freeman, 2002.

4. Murray, R.K., Granner, D.K., Mayes, P.A. and Rodwell, V.W. (2009) Harper’s

Illustrated Biochemistry. XXVIII edition. Lange Medical Books/ McGraw-Hill.

5. Berg, J.M., Tymoczko, J.L. and Stryer, L. (2006) Biochemistry, 6th Edition. W.H. Freeman and Co. (2002).

6. Wilson, K. & Walker, J. Practical Biochemistry. Cambridge University Press

(2009).

7. The Tools of Biochemistry (1977; Reprint 2011) Cooper, T.G., Wiley India Pvt. Ltd. (New Delhi), ISBN: 978-81-265-3016-8.

CORE PAPER XIV LAB

1. Preparations of the following compounds

i. Aspirin

ii. Methyl orange

2. Estimation of phenol and aniline by bromination method.

3. Saponification value of an oil/fat/ester.

4. Estimation of glycine by Sorenson’s formalin method.

5. Estimation formaldehyde (formalin).

6. Estimation of ascorbic acid in fruit juices/Vitamin C tablet (Iodometric method)


7. Determination of Iodine number of an oil/ fat.

Reference Books:

1. Arthur, I. Vogel, Elementary Practical Organic Chemistry, Part-1 Small scale preparations, Indian Edition, Pearson (2011).

2. Manual of Biochemistry Workshop, 2012, Department of Chemistry, University

of Delhi.

3. Arthur, I. Vogel, Quantitative Organic Analysis, Pearson.

4. Wilson, K. & Walker, J. Practical Biochemistry. Cambridge University Press (2009).

Discipline Specific Elective Paper-1

POLYMER CHEMISTRY

UNIT-I

Introduction and history of polymeric materials: Different schemes of classification of polymers, Polymer nomenclature, Molecular forces and chemical bonding in polymers, Texture of Polymers. Functionality and its importance: Criteria for synthetic polymer formation, classification of polymerization processes, Relationships between functionality, extent of reaction and degree of polymerization. Bi-functional systems, Poly-functional systems.

UNIT-II

Mechanism & Kinetics of Polymerization: Polymerization reactions – addition and condensation, mechanism and kinetics of step growth, radical chain growth, ionic chain (both cationic and anionic) and coordination polymerizations, Mechanism and kinetics of copolymerization, polymerization techniques. Crystallization and crystallinity: Determination of crystalline melting point and degree of crystallinity, Morphology of crystalline polymers, Factors affecting crystalline melting point.

UNIT-III

Molecular weight of polymers and their determination (Mn,Mw, Mv, Mz) by end group analysis,viscometry and osmotic pressure methods. Molecular weight distribution and its significance. Polydispersity index. Glass transition temperature (Tg) and it determination: WLFequation, Outlines of factors affecting glass transition temperature (Tg).


UNIT-IV Properties of polymers (physical, thermal and mechanical properties).

Preparation, structure, properties and applications of the following polymers: polyolefins (polyethylene, polypropylene), polystyrene, polyvinyl

chloride, polyvinyl acetate, polyacrylamide, fluoro polymers (Teflon), polyamides

(nylon-6 and nylon 6,6). Thermosetting polymers - phenol formaldehyde resins

(Bakelite, Novalac), polyurethanes, conducting polymers (polyacetylene,

polyaniline). Brief outline of biodegradable polymers.


1. V. R. Gowarikar, Jayadev Sreedhar, N. V. Viswanathan, Polymer Science 1st Edition, New Age International Publishers, 1986.

2. Premamoy Ghosh, Polymer Science and Technology: Plastics, Rubber, Blends and Composites, 3rdEdition, McGraw Hill Education, 2010.

3. P. Bahadur &N.V.Sastry, Principles of polymer science, Narosa Publishing

house, New Delhi 2002. 4. Fred W. Billmeyer, Textbook of Polymer Science, 3rd ed. Wiley-Interscience

(1984) Reference books

1. L.H. Sperling, Introduction to Physical Polymer Science, 4th ed. John Wiley & Sons (2005)

2. Malcolm P. Stevens, Polymer Chemistry: An Introduction, 3rd ed. Oxford University Press (2005)

3. Seymour/Carraher’s Polymer Chemistry, 9th ed. by Charles E. Carraher, Jr. (2013).

4. Nayak P.L., Polymer Chemistry, Kalyani Publisher (2017).

Discipline Specific Elective Paper I LAB Polymer synthesis (At least three experiment)

1. Preparation of nylon-6,6 / Polyaniline 2. Preparations of phenol-formaldehyde resin-novalac / phenol-formaldehyde

resin resold. 3. Preparation of urea-formaldehyde resin 4. Free radical solution polymerization of styrene (St) / Methyl Methacrylate

(MMA) / Methyl Acrylate (MA) / Acrylic acid (AA). a. Purification of monomer b. Polymerization using benzoyl peroxide (BPO) / 2,2’-azo-bis-isobutylonitrile

(AIBN) 5. Redox polymerization of acrylamide 6. Precipitation polymerization of acrylonitrile


Polymer characterization/analysis (At least two different experiemtn) 1. Determination of molecular weight by viscometry:

a. Polyacrylamide / Polystyrene

b. (Polyvinyl pyrolidine (PVP)

2. Determination of acid value/saponification value of a resin.

3. Determination of hydroxyl number of a polymer using colorimetric method.

4. Estimation of the amount of HCHO in the given solution by sodium sulphite

method

5. Analysis of some IR spectra of polymers – Identification of labelled peaks in IR spectra of known polymer.

Reference Books:

1. Hundiwale G.D., Athawale V.D., Kapadi U.R. and Gite V. V., Experiments in

Polymer Science, New Age Publications (2009) 2. Malcohm P. Stevens, Polymer Chemistry: An Introduction, 3rd Ed. 3. Joel R. Fried, Polymer Science and Technology, 2nd ed. Prentice-Hall (2003) 4. Petr Munk and Tejraj M. Aminabhavi, Introduction to Macromolecular Science,

2nd ed. John Wiley & Sons (2002) 5. Malcolm P. Stevens, Polymer Chemistry: An Introduction, 3rd ed. Oxford

University Press (2005).

Discipline Specific Elective Paper-1I

GREEN CHEMISTRY

UNIT-I

Introduction to Green Chemistry What is Green Chemistry? Need for Green Chemistry. Goals of Green Chemistry. Limitations/ Obstacles in the pursuit of the goals of Green Chemistry. Principles of Green Chemistry and Designing a Chemical synthesis-I Twelve principles of Green Chemistry. Explanations of principle with special

emphasis on - Designing green synthesis processes: Prevention of Waste/ by-

products; maximize the incorporation of the materials used in the process into the

final products (Atom Economy) with reference to rearrangement, addition,

substitution and elimination reactions; Prevention/ minimization of hazardous/

toxic products; Designing safer chemicals; Use of safer solvents and auxiliaries

(e.g. separating agent) - green solvents (supercritical CO2, water, ionic liquids),

solventless processes, immobilized solvents.


UNIT-II

Principles of Green Chemistry and Designing a Chemical synthesis-II Explanation of green chemistry principles with special emphasis on: Energy

efficient processes for synthesis - use of microwaves and ultrasonic energy.

Selection of starting materials (use of renewable feedstock); avoidance of

unnecessary derivatization (e.g. blocking group, protection groups, deprotection);

Use of catalytic reagents (wherever possible) in preference to stoichiometric

reagents; designing of biodegradable products use of chemically safer

substances for prevention of chemical accidents, inherent safer design greener -

alternative to Bhopal Gas Tragedy (safer route to carcarbaryl) and Flixiborough

accident (safer route to cyclohexanol); real-time, in-process monitoring and

control to prevent the formation of hazardous substances; development of green

analytical techniques to prevent and minimize the generation of hazardous

substances in chemical processes. UNIT-III

Examples of Green Synthesis/ Reactions and some real world cases-I Green Synthesis of the following compounds: adipic acid, catechol, methyl

methacrylate, urethane, disodium iminodiacetate (alternative to Strecker

synthesis), paracetamol, furfural. Microwave assisted reactions: Applications to

reactions (i) in water: Hofmann Elimination, hydrolysis (of benzyl chloride, methyl

benzoate to benzoic acid), Oxidation (of toluene, alcohols); (ii) reactions in

organic solvents: Diels-Alder reaction and Decarboxylation reaction. Ultrasound

assisted reactions: Applications to esterification, saponification, Simmons-Smith

Reaction (Ultrasonic alternative to Iodine).

UNIT-IV

Examples of Green Synthesis/ Reactions and some real world cases-II Surfactants for carbon dioxide – replacing smog producing and ozone depleting solvents with CO2 for precision cleaning and dry cleaning of garments; Designing of Environmentally safe marine antifoulant; Rightfit pigment: synthetic azopigments to replace toxic organic and inorganic pigments; Synthesis of a compostable and widely applicable plastic (poly lactic acid) from corn; Development of Fully Recyclable Carpet: Cradle to Cradle Carpeting


Future Trends in Green Chemistry

Oxidizing and reducing reagents and catalysts; multifunctional reagents; Combinatorial green chemistry; Proliferation of solventless reactions; Green chemistry in sustainable development. (Bio-diesel, bio-ethanol and biogas)


1. Anastas P.T. & Warner J.K.: Green Chemistry- Theory and Practical, Oxford University Press (2000).

2. Ahluwalia V.K. & Kidwai M.: New Trends in Green Chemistry, Anamalaya

Publishers, New Delhi (2004).

3. Kumar V., An Introduction to Green Chemistry, Vishal Publishing Co., (2015). Reference Books:

1. Matlack A.S. Introduction to Green Chemistry, Marcel Dekker (2001).

2. Das Asim K. amd Das Mahua , Environment Chemistry with Green Chemistry, Books and Allied (P) Ltd. (2010)

Discipline Specific Elective Paper II LAB

At least five experiments should be done: 1. Acetylation of primary amine (Aniline to N-phenylacetamide) using Zn dust. 2. Nitration of salicylic acid by green method (Using calcium nitrate and acetic acid). 3. Bromination of acetanilide using ceric ammonium nitrate/KBr. 4. Microwave assisted nitration of Phenols using Cu(NO3)2. 5. Detection of elements in organic compounds by green method (Sodium carbonate

fusion) 6. Base catalyzed Aldol condensation (Synthesis of dibenzalpropanone) 7. Vitamin C clock reaction using vitamin C tablets, tincture of iodine, hydrogen

peroxide and liquid laundry starch. Effect of concentration on clock reaction. 8. Photoreduction of benzophenone to benzopinacol in the presence of sunlight. 9. Diels Alder reaction in water: Reaction between furan and maleic acid in

water and at room temperature rather than in benzene and reflux. 10. Preparation and characterization of nanoparticles (Cu, Ag) using plant extract. 11. Preparation of propene by following two methods or any other reactions like

addition, elimination, substitution showing atomic economy can be studied (I) Triethylamine ion + OH- → propene + trimethylpropene + water

H2SO4/Δ

(II) 1-propanol propene + water


Reference Books: 1. Monograph on Green Chemistry Laboratory Experiments, edited and published by

Green Chemistry Task Force Committee, DST Govt. of India, p. 1-79. 2. Kirchoff, M. & Ryan, M.A. Greener approaches to undergraduate

chemistryexperiment. American Chemical Society, Washington DC (2002). 3. Sharma, R.K.; Sidhwani, I.T. & Chaudhari, M.K. I.K. Green Chemistry Experiment:A

monograph International Publishing House Pvt Ltd. New Delhi. Bangalore CISBN978-93-81141-55-7 (2013).

Discipline Specific Elective Paper-1II

INDUSTRIAL CHEMICALS AND ENVIRONMENT UNIT-I

Industrial Gases and Inorganic Chemicals Industrial Gases: Large scale production, uses, storage and hazards in handling of thefollowing gases: oxygen, nitrogen, argon, hydrogen, acetylene, carbon monoxide, chlorine, sulphur dioxide. Inorganic Chemicals: Manufacture, application and hazards in handling the following chemicals: hydrochloric acid, nitric acid, sulphuric acid, caustic soda, common salt, bleaching powder, sodium thiosulphate, hydrogen peroxide, potash alum, potassium dichromate and potassium permanganate. Industrial Metallurgy Preparation of metals (ferrous and nonferrous) and ultra pure metals for semiconductor technology.

UNIT-II Environment and its segments Ecosystems. Biogeochemical cycles of carbon, nitrogen and sulphur. Air

Pollution: Major regions of atmosphere. Chemical and photochemical reactions in

atmosphere. Air pollutants: types, sources, particle size and chemical nature;

Photochemical smog: its constituents and photochemistry. Environmental effects

of ozone. Major sources of air pollution. Pollution by SO2, CO2, CO, NOx, and

H2S and control procedures. Effects of air pollution on living organisms and

vegetation. Greenhouse effect and global warming, Ozone depletion by oxides of

nitrogen, chlorofluorocarbons and halogens, removal of sulphur from coal.


UNIT-III

Water Pollution: Hydrological cycle, water resources, aquatic ecosystems, Sources andnature of water pollutants, Techniques for measuring water pollution, Impacts of water pollution on hydrological and ecosystems. Water purification methods. Effluent treatment plants (primary, secondary and tertiary treatment). Industrial effluents from the following industries and their treatment: electroplating, textile, tannery, dairy, petroleum and petrochemicals, fertilizer. Sludge disposal. Industrial waste management: incineration of waste. Water treatment and purification (reverse osmosis, ion exchange). Water quality parameters for wastewater, industrial water and domestic water.

UNIT-IV

Energy and Environment Sources of energy: Coal, petrol and natural gas. Nuclear fusion/fission, solar energy, hydrogen, geothermal, tidal and hydel. Nuclear Pollution: Disposal of nuclear waste, nuclear disaster and its management. Biocatalysis Introduction to biocatalysis: Importance in green chemistry and chemical industry.


1. De, A. K. Environmental Chemistry: New Age International Pvt., Ltd, New Delhi, 2010.

2. Stocchi E., Industrial Chemistry, Vol-I, Ellis Horwood Ltd. UK.

3. Sharma, B.K. & Gaur, H. Industrial Chemistry, Goel Publishing House, Meerut

(1996). Reference Books:

4. Felder R.M. and Rousseau R.W., Elementary Principles of Chemical Processes, Wiley Publishers, New Delhi.

5. Dara S. S., A Textbook of Engineering Chemistry, S. Chand & Company

Ltd. New Delhi. 6. Miller G.T., Environmental Science, 11th edition. Brooks/ Cole (2006). 7. Mishra, Environmental Studies, Selective and Scientific Books, New Delhi

(2005).


Discipline Specific Elective Paper III LAB

1. Determination of Dissolved Oxygen (DO) in water.

2. Determination of Chemical Oxygen Demand (COD)

3. Determination of Biological Oxygen Demand (BOD)

4. Percentage of available chlorine in bleaching powder.

5. Measurement of chloride, sulphate and salinity of water samples by simple titration method (AgNO3 and potassium chromate).

6. Estimation of total alkalinity of water samples (CO32-, HCO3

-) using double titration method.

7. Measurement of dissolved CO2. 8. Study of some of the common bio-indicators of pollution.

9. Estimation of SPM in air samples.

10. Preparation of borax/ boric acid.

Reference Books:

1. Dara S. S., A Textbook on Experiments and Calculations in Engineering ChemistrySChand & Company; 9th Revised edition (2015).

2. E. Stocchi: Industrial Chemistry, Vol-I, Ellis Horwood Ltd. UK.

3. R.M. Felder, R.W. Rousseau: Elementary Principles of Chemical Processes, Wiley Publishers, New Delhi.

4. A. Kent: Riegel’s Handbook of Industrial Chemistry, CBS Publishers, New Delhi.

5. S. M. Khopkar, Environmental Pollution Analysis: Wiley Eastern Ltd, New Delhi.

Discipline Specific Elective Paper-IV

DISSERTATION

A project work is to be carried out by the student in consultation with the teachers of the department. The report of work (dissertation) in a standard format is to be submitted and presented for evaluation. Distribution of marks

(a) Project Report/Dissertation (Proper documentation of literature, data, discussion etc. and logical flow of work undertaken): 60 Marks

(b) Seminar/Presentation: 20 marks

(c) Viva voce: 20 marks


A brief Guidelines to Project Work: 1. Students shall undertake the project work (experimental/theoretical) related to any branch of chemistry/Chemical science under the guidance of teacher(s) from the department or jointly with teachers/research personnel of other institutes.

2. The following activities have been outlined as guidelines (not exhaustive):

• Physiochemical studies (pH, conductivity, turbidity, etc.) of different wetlands (ponds, lakes, river etc.)

• Analysis of iron in pond / tube well / river water.

• Analysis of Hardness of water samples.

• Adulteration detection activities in food stuff and other edible items.

• Extraction and preliminary characterization of useful chemicals (as far as

possible) from plants.

• Solubility, surface tension, and viscosity measurements of some solution of practical relevance, (cough syrup, soap solution, pesticides, fertilizers.. etc.)

• Pollution related activities (Industrial/Agricultural/Municipal etc.)

• Nutrition related activities, (essential metal detection in food, cereals, pulses,

fruits etc.).

• Small synthetical work (inorganic/Organic/Polymeric compounds) 2. The UG level project work is a group activity, maximum number of students being

limited to five. HOD to notify the name of teacher(s) for supervising the project work of each group. A

teacher can guide more than one group, if necessary.

4. No two groups in the same institution are permitted to do project work on the same

problem. 5. Each student shall prepare and submit the project report separately for evaluation.

Two copies of project report are required to be submitted in bound form (spiral/paperback).

6. Ordinarily the students can avail the facilities of college laboratory and library for the purpose but for special requirements the student has to bear the expenses of the project.

7. The project report shall be divided as:

Chapter I: Introduction (Introduction on the topic, review of literature, objective and scope of the work)

Chapter II: Materials and methods Chapter II: Results and discussion Chapter IV: Conclusions and Scope of future studies Chapter V: References


Reference Books:

1. M. A. Malati, An Investigative, Integrated Approach to Practical Project Work; Mid-Kent

College of Higher/Further Education, UK (October 1999); Imprint: Woodhead

Publishing; ISBN: 978-1-898563-47-1.

2. Dean, J. R., Jones, A. M., Holmes, D., Reed, R., Weyers, J. & Jones, A. (2011) Practical skills in chemistry. 2nd Ed., Prentice-Hall, Harlow.


GENERIC ELECTIVE CHEMISTRY (GE)

Generic Elective Paper I (Theory)

Unit-I

Atomic Structure Review of: Bohr’s theory and its limitations, dual behaviour of matter and radiation, de-Broglie’s relation, Heisenberg Uncertainty principle. Hydrogen atom spectra. Quantum mechanics: Time independent Schrodinger equation and meaning of various terms in it. Significance of ψ and ψ2, Schrödinger equation for hydrogen atom. Quantum numbers and their significance, shapes of s, p and d atomic orbitals, nodal planes.Rules for filling electrons in various orbitals, Electronic configurations of the atoms. Stability of half-filled and completely filled orbitals, concept of exchange energy. Relative energies of atomic orbitals, Anomalous electronic configurations.

Unit-II

Chemical Bonding and Molecular Structure Ionic Bonding: General characteristics, energy considerations.Lattice energy and

solvation energy and their importance in the context of stability and solubility of

ionic compounds. Born-Haber cycle and its applications, polarizing power and polarizability. Fajan’s rules and its applications. Covalent bonding: VB Approach: Shapes of some inorganic molecules and ions on the basis of VSEPR and hybridization with suitable examples of linear, trigonal planar, square planar, tetrahedral, trigonal bipyramidal and octahedral arrangements.. MO Approach: Rules for the LCAO method, bonding and antibonding MOs and their characteristics for s-s, s-p and p-p combinations of atomic orbitals, nonbonding combination of orbitals, MO treatment of homonuclear diatomic molecules (N2, O2) . Comparison of VB and MO approaches


Unit- III Chemical Kinetics

The concept of reaction rates. Effect of temperature, pressure, catalyst and other factors on reaction rates. Order and molecularity of a reaction. Derivation of integrated rate equations for Zero and first order reactions.. Half–life of a reaction. General methods for determination of order of a reaction. Concept of activation energy and its calculation from Arrhenius equation. Theories of Reaction Rates: Collision theory and Activated Complex theory of bimolecular reactions. Chemical Energetics Review of thermodynamics and the Laws of Thermodynamics. Important principles and definitions of thermochemistry. Concept of standard state and standard enthalpies of formations, integral and differential enthalpies of solution and dilution. Calculation of bond energy, bond dissociation energy and resonance energy from thermochemical data. Variation of enthalpy of a reaction with temperature – Kirchhoff’s equation.

Unit-IV

Fundamentals of Organic Chemistry

Physical Effects, Electronic Displacements: Inductive effect, Electromeric effect,

Resonance and hyperconjugation. Cleavage of bonds: Homolysis and

heterolysis. Structure, shape and reactivity of organic molecules: Nucleophiles

and electrophiles. Reactive Intermediates: Carbocations, Carbanions and free

radicals. Strength of organic acids and bases: Comparative study with emphasis

on factors affecting pK values. Aromaticity: Hückel’s rule.

Stereochemistry Conformations with respect to ethane, butane and cyclohexane. Interconversion

of Wedge Formula, Newmann, Sawhorse and Fischer representations. Concept

of chirality (up to two carbon atoms). Configuration: Geometrical and Optical

isomerism; Enantiomerism, Diastereomerism and Meso compounds). D and L;

cis-trans nomenclature; CIP Rules: R/ S (for one chiral carbon atoms) and E / Z

Nomenclature (for up to two C=C systems).


Recommended Text Books: 1. Lee J. D., Concise Inorganic Chemistry, Wiley India, 5thEdn., 2008. 2. Puri, Sharma, Kalia, Principles of Inorganic Chemistry, Vishal Pub. Co., 33rd ed.,

2017. 3. Shriver D. E.,Atkins P. W., InorganicChemistry, Oxford University Press,5thEdn.. 4. Huheey J. E., Keiter E. A. and Keiter R. L., Inorganic Chemistry – Principles of

structure and reactivity, , Pearson Education, 4th Ed. 2002.

5. Morrison, R. N. & Boyd, R. N., Organic Chemistry, Dorling Kindersley (India) Pvt. Ltd. (Pearson Education).

6. BhalArun & BhalB S , Advanced Organic Chemistry, 2nd Edition, S. Chand

Publisher, 2012.

7. Kalsi, P. S. Stereochemistry Conformation and Mechanism; 8thEdn, New Age International, 2015.

Reference books



3. Mallick, Madan and Tuli, S. Chand Selected Topic in Inorganic Chemistry, , 17thEdn. 2010.


Generic Elective Paper I LAB

Section A: Inorganic Chemistry

Volumetric Analysis

1. Estimation of sodium carbonate and sodium hydrogen carbonate present in a

mixture. 2. Estimation of oxalic acid by titrating it with KMnO4. 3. Estimation of water of crystallization in Mohr’s salt by titrating with KMnO4. 4. Estimation of Fe(II) ions by titrating it with K2Cr2O7 using internal indicator. 5. Estimation of Cu(II) ions iodometrically using Na2S2O3.

6. Qualitative analysis of inorganic slat mixture using H2S: not more than four ionic species (two anions and two cations and excluding insoluble salts) out of the following: 7. 8. Cations : NH4

+, Pb2+, Ag+, Bi3+, Cu2+, Cd2+, Sn2+, Fe3+, Al3+, Co2+, Cr3+, Ni2+, Mn2+, Zn2+, Ba2+, Sr2+, Ca2+, K+

9. Anions: CO32–, S2–, SO3

2–, NO3–, Cl–, Br–, I–, NO3

–

,SO42- , PO4

3-, F-


Reference Books:

1. Mendham, J., A. I. Vogel’s Quantitative Chemical Analysis 6th Ed., Pearson, 2009.


3. Ahluwalia, V.K., Dhingra, S. and Gulati A, College Practical Chemistry, University

Press (2005).

Generic Elective Paper II (Theory) Unit-I

Chemical Equilibrium Free energy change in a chemical reaction. Thermodynamic derivation of the law of chemical equilibrium. Distinction between ΔG and ΔGo, Le Chatelier’s principle. Relationships between Kp, Kc and Kx for reactions involving ideal gases Ionic Equilibria Strong, moderate and weak electrolytes, degree of ionization, factors affecting

degree of ionization, ionization constant and ionic product of water. Ionization of

weak acids and bases, pH scale, common ion effect. Salt hydrolysis-calculation

of hydrolysis constant, degree of hydrolysis and pH for different salts. Buffer

solutions. Solubility and solubility product of sparingly soluble salts – applications

of solubility product principle.

Unit- II Aliphatic Hydrocarbons Functional group approach for the following reactions (preparations & reactions) to be studied in context to their structure. Alkanes: (Up to 5 Carbons).Preparation:Catalytic hydrogenation, Wurtz reaction,Kolbe’s synthesis, from Grignard reagent. Reactions: Free radical Substitution: Halogenation. Alkenes: (Up to 5 Carbons)Preparation:Elimination reactions: Dehydration of alkenesand dehydrohalogenation of alkyl halides (Saytzeff’s rule); cis-alkenes (Partial catalytic hydrogenation) and trans-alkenes (Birch reduction). Reactions: cis-addition (alk. KMnO4) and trans-addition (bromine), Addition of HX (Markownikoff’s and anti-Markownikoff’s addition), Hydration, Ozonolysis, Alkynes: (Up to 5 Carbons)Preparation:Acetylene from CaC2and conversion intohigher alkynes; Acidic nature of Acetylene. Aromatic hydrocarbons Preparation benzene : from phenol ( by decarboxylation),and from benzene sulphonic acid. Reactions: of benzene : Electrophilic substitution: nitration,

halogenation and sulphonation. Friedel-Craft’s reaction (alkylation and acylation)


Unit-III Alkyl and Aryl Halides Alkyl Halides (Up to 5 Carbons) : Preparation: from alkenes and alcohols. Reactions : Nucleophilic Substitution (SN1, SN2 and SNi) reactions. Aryl Halides Preparation: (Chloro, bromo and iodo-benzene case): from phenol, Sandmeyer &Gattermann reactions. Reactions (Chlorobenzene): Aromatic nucleophilic substitution Benzyne Mechanism: KNH2/NH3 (or NaNH2/NH3). Alcohols and Phenols (Up to 5 Carbons) Alcohols: Preparation: Preparation of 1°, 2° and 3° alcohols: using Grignard reagent, Ester hydrolysis, Reduction of aldehydes and ketones, carboxylic acid and esters. Reactions: With sodium, HX (Lucas test), esterification, oxidation (with PCC, alk. KMnO4, acidic dichromate, conc. HNO3). Phenols: (Phenol case) Preparation: Cumene hydroperoxide method, from diazonium salts. Reactions: Electrophilic substitution: Nitration, halogenation and sulphonation. ReimerTiemann Reaction, Gattermann-Koch Reaction,

Unit-IV

Aldehydes and ketones (aliphatic and aromatic): Formaldehyde, acetaldehyde, acetone and benzaldehyde Preparation: from acid chlorides and from nitriles. Reactions – Reaction with HCN, ROH, NaHSO3, NH2-G derivatives. Iodoform test. Aldol Condensation, Cannizzaro’s reaction, Benzoin condensation. Carboxylic Acid (aliphatic and aromatic) : Formic acid , Acetic acid and benzoic acid.Preperation by hydrolysis and oxidation, from Grignards reagent. Strength of aliphatic and aromatic carboxylic acid. Acetoacetic ester . Preperation and synthetic applications.



2. Principles of Physical Chemistry, Puri, Sharma &Pathania, Vishal Publishing Co, 47th Edn., 2017.

3. K. L. Kapoor, Text Book of Physical Chemistry, Mac Grow Hill, 3rdEdn. 2017. 4. Morrison, R. N. & Boyd, R. N., Organic Chemistry, Dorling Kindersley (India) Pvt.

Ltd. (Pearson Education).

5. Arun Bahl & B S Bahl, Advanced Organic Chemistry, 2nd Edition, S. Chand Publisher, 2012.


Reference Books:

1. Kheterpal S.C., Pradeep’s Physical Chemistry, Vol. I & II, Pradeep Publications.

2. Dhawan, S.N., Pradeep’s Organic Chemistry, (Vol. I and II), Pradeep

Publications

Generic Elective Paper II LAB

Section A: Physical Chemistry Ionic equilibria pH measurements a) Measurement of pH of different solutions like aerated drinks, fruit juices,

shampoos and soaps (use dilute solutions of soaps and shampoos to prevent damage to the glass electrode) using pH-meter.

b) Preparation of buffer solutions:

• Sodium acetate-acetic acid

• Ammonium chloride-ammonium hydroxide

Measurement of the pH of buffer solutions and comparison of the values with theoretical values.

Section B: Organic Chemistry

1 Detection of extra elements (N, S, Cl) in organic compounds (containing up to two extra elements)

2 Preparations, recrystallisation, determination of melting point and calculation of quantitative yields of the followings:

(e) Bromination of Phenol/Aniline

(f) Benzoylation of amines/phenols

(g) Oxime and 2,4 dinitrophenylhydrazone of aldehyde/ketone

Reference Books

1. A.I. Vogel: Textbook of Practical Organic Chemistry, 5th edition, Prentice-

Hall.

2. Mann, F.G. & Saunders, B.C. Practical Organic Chemistry, Pearson Education (2009).

3. Ahluwalia, V.K., Dhingra, S. and Gulati A, College Practical Chemistry,

University Press (2005).

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